Input interpretation
![HNO_3 nitric acid + Na sodium ⟶ H_2O water + NO_2 nitrogen dioxide + Na_2O sodium oxide](../image_source/e6c9ca9b9afbca244984ccb5c199e631.png)
HNO_3 nitric acid + Na sodium ⟶ H_2O water + NO_2 nitrogen dioxide + Na_2O sodium oxide
Balanced equation
![Balance the chemical equation algebraically: HNO_3 + Na ⟶ H_2O + NO_2 + Na_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Na ⟶ c_3 H_2O + c_4 NO_2 + c_5 Na_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Na: H: | c_1 = 2 c_3 N: | c_1 = c_4 O: | 3 c_1 = c_3 + 2 c_4 + c_5 Na: | c_2 = 2 c_5 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HNO_3 + 2 Na ⟶ H_2O + 2 NO_2 + Na_2O](../image_source/6ca974b5e14c41933b8b8fbd0daf1c0d.png)
Balance the chemical equation algebraically: HNO_3 + Na ⟶ H_2O + NO_2 + Na_2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HNO_3 + c_2 Na ⟶ c_3 H_2O + c_4 NO_2 + c_5 Na_2O Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O and Na: H: | c_1 = 2 c_3 N: | c_1 = c_4 O: | 3 c_1 = c_3 + 2 c_4 + c_5 Na: | c_2 = 2 c_5 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_3 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 2 c_3 = 1 c_4 = 2 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HNO_3 + 2 Na ⟶ H_2O + 2 NO_2 + Na_2O
Structures
![+ ⟶ + +](../image_source/038fd5959cf74958c6f4581e20b3595d.png)
+ ⟶ + +
Names
![nitric acid + sodium ⟶ water + nitrogen dioxide + sodium oxide](../image_source/dfe47749c6ffb63194497fabbc9eaf6d.png)
nitric acid + sodium ⟶ water + nitrogen dioxide + sodium oxide
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HNO_3 + Na ⟶ H_2O + NO_2 + Na_2O Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: 2 HNO_3 + 2 Na ⟶ H_2O + 2 NO_2 + Na_2O Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i HNO_3 | 2 | -2 Na | 2 | -2 H_2O | 1 | 1 NO_2 | 2 | 2 Na_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) Na | 2 | -2 | ([Na])^(-2) H_2O | 1 | 1 | [H2O] NO_2 | 2 | 2 | ([NO2])^2 Na_2O | 1 | 1 | [Na2O] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([HNO3])^(-2) ([Na])^(-2) [H2O] ([NO2])^2 [Na2O] = ([H2O] ([NO2])^2 [Na2O])/(([HNO3])^2 ([Na])^2)](../image_source/a2accb8fdd2dc5c3812cdd2d521117e2.png)
Construct the equilibrium constant, K, expression for: HNO_3 + Na ⟶ H_2O + NO_2 + Na_2O Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: 2 HNO_3 + 2 Na ⟶ H_2O + 2 NO_2 + Na_2O Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i HNO_3 | 2 | -2 Na | 2 | -2 H_2O | 1 | 1 NO_2 | 2 | 2 Na_2O | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HNO_3 | 2 | -2 | ([HNO3])^(-2) Na | 2 | -2 | ([Na])^(-2) H_2O | 1 | 1 | [H2O] NO_2 | 2 | 2 | ([NO2])^2 Na_2O | 1 | 1 | [Na2O] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([HNO3])^(-2) ([Na])^(-2) [H2O] ([NO2])^2 [Na2O] = ([H2O] ([NO2])^2 [Na2O])/(([HNO3])^2 ([Na])^2)
Rate of reaction
![Construct the rate of reaction expression for: HNO_3 + Na ⟶ H_2O + NO_2 + Na_2O Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: 2 HNO_3 + 2 Na ⟶ H_2O + 2 NO_2 + Na_2O Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i HNO_3 | 2 | -2 Na | 2 | -2 H_2O | 1 | 1 NO_2 | 2 | 2 Na_2O | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) Na | 2 | -2 | -1/2 (Δ[Na])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO_2 | 2 | 2 | 1/2 (Δ[NO2])/(Δt) Na_2O | 1 | 1 | (Δ[Na2O])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -1/2 (Δ[HNO3])/(Δt) = -1/2 (Δ[Na])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[NO2])/(Δt) = (Δ[Na2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/df9b831e2b98491130a7ddb4febfcb90.png)
Construct the rate of reaction expression for: HNO_3 + Na ⟶ H_2O + NO_2 + Na_2O Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: 2 HNO_3 + 2 Na ⟶ H_2O + 2 NO_2 + Na_2O Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i HNO_3 | 2 | -2 Na | 2 | -2 H_2O | 1 | 1 NO_2 | 2 | 2 Na_2O | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term HNO_3 | 2 | -2 | -1/2 (Δ[HNO3])/(Δt) Na | 2 | -2 | -1/2 (Δ[Na])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) NO_2 | 2 | 2 | 1/2 (Δ[NO2])/(Δt) Na_2O | 1 | 1 | (Δ[Na2O])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -1/2 (Δ[HNO3])/(Δt) = -1/2 (Δ[Na])/(Δt) = (Δ[H2O])/(Δt) = 1/2 (Δ[NO2])/(Δt) = (Δ[Na2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| nitric acid | sodium | water | nitrogen dioxide | sodium oxide formula | HNO_3 | Na | H_2O | NO_2 | Na_2O name | nitric acid | sodium | water | nitrogen dioxide | sodium oxide IUPAC name | nitric acid | sodium | water | Nitrogen dioxide | disodium oxygen(-2) anion](../image_source/006da381a0d9da000633f6ebe861af6e.png)
| nitric acid | sodium | water | nitrogen dioxide | sodium oxide formula | HNO_3 | Na | H_2O | NO_2 | Na_2O name | nitric acid | sodium | water | nitrogen dioxide | sodium oxide IUPAC name | nitric acid | sodium | water | Nitrogen dioxide | disodium oxygen(-2) anion